Chemistry

Copper and lead had different densities. Sketch a diagram at the particular nature of matter level showing the atoms of a small cross section of copper and lead. Use this diagram to explain why lead is denser than copper.

I couldn't find any pictures or see anywhere in my textbook about the structures of Cu and Lead, so I was wondering how it would look.
But would this be a right answer to the second part of the answer:
Lead is more denser than copper due to the atoms being packed together closer than those in copper.

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1. Nope: Lead atoms and copper atoms pack about the same, with the exception that lead has a greater atomic radius than copper (.175nm vs .128), which when cubed gives a volume ratio of (.175/.128)^3 or 2.5. The atomic mass of Pb is 207 vs Cu 63, so the ratio of mass to is 207/63= 3.3
or comparing the mass density of ocupied atomic volme is 3.3/2.5= 1.32

Now the observed density of lead is about 11.3, and the density of Cu is
atomsLead/cm^3= density 8.94, or a ratio of 11.3/8.9 = 1.27 WHICH IS ALMOST THE SAME as the density of the atomic volumes. Bottom line: the packing is nearly the same, the differences in density is due to atomic mass and atomic radius.

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2. Then if I sketch a diagram of a cross section of the atoms of both elements, it would look the same. If they look the same then in my explanation should I say, since both diagrams are the same, the only reason that lead is denser than copper is due to the fact that lead has a bigger atomic radius and mass than copper.

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3. I agree with that.

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4. So if I were to draw the cross section would I just draw it as so-

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